Name _______________________________
Period ______
Acids and Bases Worksheet
1. Identify the following as properties of
acids, bases, or both.
a. bitter ___base____________________
b. sour ____acid____________________
c. may conduct electricity __both______
d. slippery ___base_________________
e. reacts with metals while producing
hydrogen gas ___acid_____________
f. neutralized by an acid to produce salt
and water ___base________________
g. turns pH paper red ___acid_________
h. turns pH paper blue ___base________
2. The concentration of hydrogen ion in a
solution is measured to be 1.0 x 10-4 M.
a. What is the hydroxide ion
concentration?
1.0 x 10-10 M
b. What is the pH of the solution?
4.0
c. Is the solution acidic or basic?
acidic
3. The concentration of hydrogen ion in a
solution is measured to be 1.0 x 10-9 M.
a. What is the hydroxide ion
concentration?
1.0 x 10-5 M
b. What is the pH of the solution?
9
c. Is the solution acidic or basic?
basic
4. The concentration of hydrogen ion in a
solution is measured to be 3.2 x 10-11 M.
a. What is the hydroxide ion
concentration?
3.1 x 10-4 M
b. What is the pH of the solution?
10.49
c. Is the solution acidic or basic?
basic
5. The concentration of hydrogen ion in a
solution is measured to be 0.016 M.
a. What is the hydroxide ion
concentration?
6.3 x 10-13
b. What is the pH of the solution?
1.80
c. Is the solution acidic or basic?
acidic
6. Label these solutions as acidic, neutral,
basic.
a. pH = 2.6 ___acidic________________
b. pH = 7.0 ___neutral_______________
c. pH = 10.5 __basic________________
d. [H+] = 3.2 x 10-2 M ___acidic________
e. [H+] = 1.0 x 10-7 M ___neutral_______
f. [OH-] = 5.7 x 10-5 M __basic________
g. [OH-] = 2.2 x 10-10 M _acidic________
7. What is the definition of an acid?
An acid is a hydrogen ion donor.
8. What is the definition of a base?
A base is a hydrogen ion acceptor, or a
hydroxide ion donor.
9. Circle the acidic hydrogen or hydrogens in
the following acids. Example: HCl
a. HBr
b. HNO3
c. H2SO4
d. CH3CO2H
e. HCO2H
f. H2CO3
g. H2NCH2CO2H
14. Calculate the hydrogen ion concentration
from the following pH values. Identify the
solution as acidic, neutral or basic.
10. Circle the atom which is the hydrogen ion
acceptor in the following bases.
a. NaOH
a. A N B pH = 7.0 ___1.0 x 10-7_______
b. KOH
b. A N B pH = 2.7 ___2.0 x 10-3_______
c. Mg(OH)2
c. A N B pH = 13.0 __1.0 x 10-13______
d. NH3
e. CH3NH2
15. Write equations showing how each
substance produces either H+ or OH–. Label
the substance as an acid or a base.
Example: A B HCO2H → H+ + HCO2–
a. A B HCl → H+ + Cl–
b. A B HNO3 → H+ + NO3–
c. A B H2SO4 → 2H+ + SO42–
d. A B H2CO3 → 2H+ + CO32–
e. A B KOH → K+ + OH–
f. A B Ca(OH)2 → Ca2+ + 2OH–
g. A B NH3 + H2O → NH4+ + OH–
h. A B HCO2H → H+ + HCO2–
i. A B CH3CO2H → H+ + CH3CO2–
j. A B CH3NH2 + H2O →
CH3NH3+ + OH–
f. H2NCH2CO2H
11. Which reaction is equivalent to:
HIO3 + H2O → H3O+ + IO3–
a. HIO3 → H+ + IO3–
b. HIO3 + H2O → H+ + IO3–
c. HIO3 → H3O+ + IO3–
d. HIO3 + H3O+ → H2O + IO3–
12. Write the chemical reaction which shows
how ammonia produces hydroxide ion.
NH3 + H2O → NH4+ + OH–
13. Calculate the pH of the following solutions
and label the solutions as acidic, neutral or
basic by circling the letter A, N or B.
a. A N B [H+] = 1.0 x 10-2 M ___2.00___
+
16. Complete the following reactions. Make
sure the equations are balanced.
Example: HCl + NaOH → NaCl + H2O
-7
b. A N B [H ] = 1.0 x 10 M ___7.00___
a. H2SO4 + Mg(OH)2 → MgSO4 + 2H2O
c. A N B [H+] = 1.0 x 10-9 M ___9.00___
d. A N B [H+] = 2.7 x 10-5 M ___4.57___
b. CH3CO2H + NaOH →
CH3CO2Na + H2O
e. A N B [H+] = 7.0 x 10-7 M ___6.15___
f. A N B [H+] = 1.0 M ________0.00___
c. HCl + NaHCO3 → NaCl + H2CO3
+
g. A N B [H ] = 0.15 M _______0.82___
d. CH3NH2 + HCl → CH3NH3Cl
h. A N B [OH-] = 5.7 x 10-5 M __9.76__
i. A N B [OH-] = 2.2 x 10-10 M _4.34___
e. H2NCH2CO2H + HCl →
H3NCH2CO2HCl
j. A N B [OH-] = 1.0 x 10-7 M __7.00__
k. A N B [OH-] = 1.0 x 10-14 M _0.00___
f. H2NCH2CO2H + NaOH →
H2NCH2CO2Na + H2O
l. A N B [OH-] = 1.0 M ______14.00___
m. A N B [OH-] = 0.050 M ____12.70___
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